1332 CHAPTER 18 Sample Questions
|
|
- Hollie Merritt
- 7 years ago
- Views:
Transcription
1 1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) V AuCl 4 + 3e Au + 4Cl V Ag + + e Ag V Hg e 2 Hg V Fe 3+ (aq) + e Fe 2+ (aq) V Cu 2+ (aq) + 2e Cu(s) V Cd 2+ (aq) + 2e Cd(s) 0.40 V Fe e Fe V Zn e Zn 0.76 V Mn e Mn 1.18 V Al e Al V Mg e Mg V REDOX 1. What is the oxidation number of phosphorus in H 3 PO 2? In the ion H 2 P 2 O 7 2, the oxidation number for P is In which acid is the oxidation number of phosphorus lowest? H 4 P 2 O 7 H 3 PO 4 PH 3 H 3 PO 3 4. Identify the pair of compounds having underlined atoms with the same oxidation number. H 2 SO 4 and HMnO 4 HClO 3 and HNO 2 HClO 4 and H 2 Cr 2 O 7 HNO 3 and H 3 PO 4 5. The oxidation number of Cl in KClO 2 is +1 l What is the oxidation number of sulfur in S 2 O 6 2? Which statement is true for the reaction - Fe(s) + Cu 2+ (aq) Cu(s) + Fe 2+ (aq) Cu 2+ is oxidized. Cu 2+ gains in oxidation state. Cu 2+ is reduced. Fe(s) is reduced. 8. Consider the reaction, 2Fe 3+ (aq) + 2I (aq) 2Fe 2+ (aq) + I 2 (aq). Which statement is true: Fe 3+ is oxidized. Fe 3+ increases in oxidation number. Fe 3+ is reduced. I is reduced. 1
2 9. In the chemical reaction, Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s), metallic zinc is the reducing agent. metallic zinc is reduced. copper ion is oxidized. sulfate ion is the oxidizing agent. 10. Which substance behaves as the oxidizing agent in Pb + PbO 2 + 2H 2SO 4 2PbSO 4 + 2H 2O Pb PbSO 4 PbO 2 H 2 SO In the process of oxidizing Fe 2+ to Fe 3+, Cr 2 O 7 2 is reduced to Cr 3+. How many moles of Fe 2+ are oxidized by one mole of Cr 2 O 7 2? Given the unbalanced equation, ClO 3 + NO 2 Cl + NO 3. How many moles of NO 2 will react with l mol of ClO 3? l Balance this equation, Fe 2+ + MnO 4 Fe 3+ + MnO 2 (in basic solution) The sum of the total number of moles on the left side of the balanced equation is 7 mol 6 mol 5 mol 4 mol 14. Balance the equation for this reaction carried out in a basic solution: CrO HSnO 2 HSnO 3 + CrO 2. The coefficient of HSnO 2 will be l What is the coefficient of Br when this equation is completed and balanced using the smallest integer coefficients? Br (aq) + MnO 4 (aq) Br 2 (l) + Mn 2+ (aq) (acidic solution) In acidic aqueous solution, MnO 4 reacts with Fe 2+ to give Mn 2+ and Fe 3+. Complete and balance the equation. What is the coefficient of Fe 2+ in the overall net ionic equation? l Complete and balance the equation assuming the reaction is carried out in basic, aqueous solution, MnO 4 (aq) + S 2 (aq) MnO 2 (s) + S(s). What is the coefficient for water? In acidic, aqueous solution Cr 2 O 7 2 reacts with H 2 S to give S(s) and Cr 3+ (aq). When the equation is balanced, the coefficient of the H + (aq) in the overall net ionic equation is
3 19. Balance ClO 4 + Fe 2+ ClO + + Fe 3+ in acidic solution. The coefficient of H + ions is: (E) Balance the equation for this reaction. Cr 2 O HSO 3 Cr 3+ + SO 4 2 in acidic solution. What number appears before H 2 O? (E) Balance the ionic equation for this reaction: MnO 4 + H 2 O 2 Mn 2+ + O 2 (in acidic solution). What is the coefficient for H 2 O 2? l (E) The sum of all coefficients when the equation MnO 4 + Cl Mn 2+ + Cl 2 (in acid) is balanced is: (E) 51 E values 23. What would be the E 0 value in volts for a zinc silver galvanic cell? What is the E 0 value for a cadmium silver voltaic cell? 0.6 V 2.0 V 1.2 V 0.40 V 25. What is the value of E 0 for the spontaneous reaction resulting from a suitable combination of these halfreactions? Fe 3+ + e Fe V Hg e 2 Hg V V V V V (E) 1.56 V 26. In a galvanic (voltaic) cell in which the reaction is, Cd + Cu 2+ Cu + Cd 2+, and the ions are at unit concentration (activity), the cell potential is 0.14 V 0.40 V 0.34 V 0.74 V (E) 0.37 V 27. What is E 0 for this reaction, 3Mn + 2AuCl 4 3Mn Au + 8Cl 0.18 V 2.18 V V 5.54 V 28. If E for the reaction Br 2 (l) + 2Ce 3+ (aq) 2Br (aq) + 2Ce 4+ (aq) is 0.55, what is E for Ce 4+ (aq) + e Ce V 0.04 V 0.51 V V 3
4 29. Using the following half-reactions, select the strongest reducing agent: HgO + H 2 O + 2e - Hg + 2 OH - Zn(OH) 2 + 2e - Zn + 2 OH - Ag 2 O + H 2 O + 2e - Ag + 2 OH - B(OH) H + + 9e - - BH H2 O E = V E = V E = V E = V Hg Zn Ag BH In the cell shown, which reaction occurs at the cathode? Cu(s) Cu 2+ (aq) Ag + (aq) Ag(s) Cu 2+ (aq) + 2 e - Cu(s) Ag(s) Ag + (aq) + e - Ag + (aq) + e - Ag(s) Cu(s) Cu 2+ (aq) + 2 e - (E) none of these 31. What is the E cell for a voltaic cell that operates using the half reactions below? Cu e - Cu(s) E = 0.34 V Sn e - Sn(s) E = 0.13 V 0.68 V 0.47 V V 0.21 V (E) V 32. The iodine clock reaction [S 2 O 8 2- (aq) + 2 H + (aq) + 2 I - (aq) 2 HSO 4 - (aq) + I 2 (aq)] has E = V and the reduction potential for I e - 2 I - = V. What is the reduction potential of S 2 O 8 2-? V V V V (E) V 33. Given the standard reduction potentials for the following half-reactions, Pb 2+ /Pb = V and Ni 2+ /Ni = V; which substance would be oxidized in a voltaic cell? Pb 2+ H + Ni Pb (E) Ni Which pair of substances will produce the greatest electromotive force when used as electrodes in 1 M solutions of their ions given the reactivity series? Na > Zn > Fe > Pb > H > Cu > Hg > Ag sodium and pure mercury iron and pure mercury sodium and hydrogen iron and copper (E) zinc and hydrogen 35. Using only the metals Mg, Al, Zn, Fe, Cu and Ag, together with their l M salt solutions, a voltaic cell of the highest possible voltage would be constructed using electrodes of these metals: Mg and Ag Mg and Fe Zn and Cu Al and Ag (E) Mg and Al 4
5 36. Using the potentials given at the start as well as the fact that Ce 4+ + e - Ce 3+ is V, determine which of the following reactions will be spontaneous under standard conditions. copper reduces silver ions ferrous ions reduce zinc ions bromide ions reduce zinc ions bromine oxidizes cerium(iii) ions Cells 37. In every electrolytic and galvanic (voltaic) cell the anode is that electrode at which oxidation occurs. which attracts cations. at which electrons are supplied to the solution. at which reduction occurs. 38. Which statement is true for the cell as it discharges, Zn Zn 2+ (1.0 M) Sn 2+ (1.0 M) Sn Oxidation occurs at the tin electrode. Electrons will flow from the tin electrode to the zinc electrode. The concentration of Zn 2+ will increase. The mass of the tin electrode will decrease. 39. In every electrolytic and galvanic cell, the cathode is the electrode which attracts cations which attracts anions at which oxidation occurs at which reduction occurs (E) at which electrons are removed to the solution 40. Two types of electrochemical cells, voltaic and electrolytic, can be described. Which statement about them is TRUE? (E) current flows directly from the cathode to the anode in an electrolytic cell the anode in a voltaic cell will gain weight as it runs oxidation occurs at the cathode in a voltaic cell the free energy change, ΔG, is negative for voltaic cells the potential of voltaic cells is independent of concentration Spontaneity etc 41. Which reaction is spontaneous in the direction written? 2Ag + Cu 2+ Cu + 2Ag + Fe + Zn 2+ Fe 2+ + Zn 2Al + 3Mg 2+ 2Al Mg 2Al + 3Zn 2+ 2Al Zn 42. A spontaneous electrochemical reaction has: ΔG = 0, E = 0, and K >> 1 ΔG < 0, E > 0, and K > 1 ΔG > 0, E < 0, and K < 1 ΔG > 0, E < 0, and K > 1 (E) ΔG < 0, E = 0, and K >> 1 5
6 43. Under which of the following conditions will a cell do the most work? Q/K < 1 Q/K = 1 E < 0 E = 0 (E) Q/K > Calculate K, the equilibrium constant for the reaction, Ag + (aq) + Fe 2+ (aq) Ag(s) + Fe What is the value of the equilibrium constant for the reaction between Sn 2+ and Fe(s) at 25 C given that: Sn 2+ (aq) + Fe(s) Sn(s) + Fe 2+ (aq); E = 0.30 V 1.4 x x x 10-6 (E) 7.3 x The value of E for the cell Cr(s) Cr 3+ (aq) Hg 2 2+ (aq) Hg(l) is 1.59 V. What is ΔG for the reaction at 25 C? -767 kj -460 kj -921 kj +767 kj (E) -307 kj 47. For the half-cell Pb e - Pb, E = V. What is the value of ΔG for the reaction, Pb(s) + 2 H + (aq) Pb 2+ (aq) + H 2 (g)? 12 kj kj 25 kj -25 kj (E) -12 kj 48. Calculate ΔG in kj for the reaction, Ag + (aq) + Fe 2+ (aq) Ag(s) + Fe Nernst Equation 49. Consider the equation, Cu 2+ (aq) + Fe(s) Cu(s) + Fe 2+ (aq). The standard potential for this reaction is 0.78 V. What is the potential if the concentrations are M Cu 2+ and 0.40 M Fe 2+? 0.72 V 0.75 V 0.81 V 0.84 V 50. Calculate the value of E for the cell at 25 C: Cu Cu 2+ (1.00 M) Ag + ( M) Ag A voltaic cell consists of an Mn/Mn 2+ electrode (E red = V) and a Fe/Fe 2+ electrode (E red = V). Calculate [Fe 2+ ] if [Mn 2+ ] = M and E cell = 0.78 V 0.24 M 1.1 M 1.8 M 0.80 M (E) M 52. The value of E for the reaction Pb 2+ (aq) + Zn(s) Zn 2+ (aq) + Pb(s) is 0.63 V. What is the value of E cell at 25 C when [Zn 2+ ] = M and the concentration of Pb 2+ = 1.0 M? 0.52 V 1.62 V 0.74 V 0.85 V (E) 0.41 V 6
7 53. The value of E for the reaction, Zn(s) + Cu 2+ (aq) Zn 2+ (aq) + Cu(s), is 1.10 V. What is the value of E for a cell in which [Cu 2+ ] = 1.0 x 10-5 M and [Zn 2+ ] = 1.0 M? 0.95 V 1.40 V 1.25 V 1.10 V (E) 0.80 V 54. What is the value of E for the cell, Al Al 3+ (0.500 M) Fe 3+ (0.421 M), Fe 2+ (1.0 x 10-3 M) Pt? 2.43 V 2.37 V 2.49 V 2.59 V Electrolysis 55. During electrolysis (E) positive ions gain electrons at the anode. negative ions lose electrons at the cathode. electrons enter the electrolytic cell at the cathode. ions enter the external or wired circuit and flow from plus to minus. oxidation takes place at the cathode. 56. During the electrolysis of an aqueous solution of CuSO 4 with inert electrodes (E) the anode loses mass and the cathode gains mass. the mass of the anode remains the same but the cathode gains mass. the mass of the anode decreases but the mass of the cathode remains constant. the anode and the cathode neither gain nor lose mass. both electrodes gain in mass. 57. Aqueous solutions of fluorides are difficult to oxidize at the anode of an electrolytic cell because (E) the aqueous solutions of fluorides are nonconducting. it is impossible to find the proper material from which to build the electrodes. the fluorides are not very soluble. in salts the fluoride ion has a plus charge. oxygen is released from water in preference to fluorine. 58. In the electrolysis of dilute H 2 SO 4, reduction occurs at the anode. the anode reaction is 2H + + 2e H 2 the anode reaction is 4OH O 2 + 4H + + 4e. the anode reaction is 2H 2 O 4H + + O 2 + 4e. 59. During the electrolysis of an aqueous solution of K 2 SO 4 the solution around the cathode becomes acidic. becomes more dilute. becomes basic. remains unchanged. (E) remains neutral 60. What product forms at the anode during the electrolysis of molten lithium iodide? Li + (l) Li(l) I - (l) I 2 (g) 7
8 61. Five metals are represented by the symbols L, M, T, R, and Z. When a solution containing all five ions at 1 M concentration is electrolyzed with a small applied voltage, which metal is most likely to be deposited first on the cathode? L L e 0.76 V R R e 0.34 V M M e 0.44 V T T e 0.13 V Z Z + + e 0.80 V L M T R (E) Z 62. The half-reaction that occurs at the cathode during the electrolysis of molten sodium bromide is: Br e - 2 Br - 2 Br - Br e - Na Na + + e - 2 H 2 O + 2 e - 2 OH - + H 2 (E) Na + + e - Na 63. Which requires the smallest voltage for electrolytic deposition given the reactivity order: Na > Al > Zn > Fe > Cu Na + Al 3+ Fe 2+ Zn 2+ (E) Cu How many coulombs of electricity are required to convert g of AgNO 3 into metallic Ag? A solution of CdSO 4 is electrolyzed between inert electrodes. How many hours must a current of 1.75 A flow to deposit 11.8 g of cadmium? Chromium metal can be plated from an acidic solution of CrO 3. How many grams of chromium will be plated by the passage of 19,300 C (coulombs)? What time is required to plate 2.08 g of copper from Cu 2+ at a constant current flow of 1.26 A? 41.8 min 128 min 83.6 min 5013 min 68. Nickel is a transition element and has a variable valence. Using a nickel salt, 2 F (faradays) plate out 39.2 g of nickel. What ions are in the solution of this salt? Ni + Ni 2+ Ni 3+ Ni 2/ A given amount of electric charge deposits g of silver from an Ag + solution. What mass of copper from a Cu 2+ solution will be deposited by the same quantity of electric charge? g 1.97 g 2.54 g 127 g 8
9 70. How many grams of aluminum are deposited from AlCl 3 in 30 min by a current of 40 A? 3.0 g 6.7 g 9.0 g 13.5 g (E) 27.0 g 71. One liter of solution contains 32.0 g of Cr(NO 3 ) 2. What current would be used to deposit all of the chromium in 5.0 h? 0.72 A 1.4 A 1.9 A 9.9 A 72. An aqueous copper(ii) sulfate solution is electrolyzed for 45 minutes using a 3.2 amp current. What mass of copper is produced? 5.6 g 0.95 g 1.9 g 2.8 g (E) 4.6 g 73. An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 2.50 amperes passing for 50.0 minutes. Reduction of ruthenium ions deposits g of Ru metal at the cathode. What was the charge on the ruthenium ions in the solution? (E) Calculate the quantity of charge necessary to produce 10 liters of H 2 (g) at STP from the electrolysis of water. 8.6 x 10 4 C 1.7 x 10 4 C 5.3 x 10 4 C 4.8 x 10 4 C (E) 3.7 x 10 4 C 75. How many grams of Ca metal can be produced by the electrolysis of molten CaBr 2 using a current of 30.0 A for 10.0 hours? g 448 g 112 g 22.4 g (E) 224 g ANSWERS: A C C D C B C C A C D C B C D C D C D B C D C C A D C D B C D A C A A A A C D D D B A C A C D D B B B C A D C B E D C D E E E C C C C C A B C D D A E 9
Electrochemistry - ANSWERS
Electrochemistry - ANSWERS 1. Using a table of standard electrode potentials, predict if the following reactions will occur spontaneously as written. a) Al 3+ + Ni Ni 2+ + Al Al 3+ + 3e - Al E = -1.68
More information2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
More informationK + Cl - Metal M. Zinc 1.0 M M(NO
Redox and Electrochemistry This section should be fresh in your minds because we just did this section in the text. Closely related to electrochemistry is redox chemistry. Count on at least one question
More informationCh 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chemistry 1C-Dr. Larson Chapter 20 Review Questions MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) is reduced in the following reaction: Cr2O7
More informationElectrochemistry Voltaic Cells
Electrochemistry Voltaic Cells Many chemical reactions can be classified as oxidation-reduction or redox reactions. In these reactions one species loses electrons or is oxidized while another species gains
More informationChem 1721 Brief Notes: Chapter 19
Chem 1721 Brief Notes: Chapter 19 Chapter 19: Electrochemistry Consider the same redox reaction set up 2 different ways: Cu metal in a solution of AgNO 3 Cu Cu salt bridge electrically conducting wire
More informationCHAPTER 21 ELECTROCHEMISTRY
Chapter 21: Electrochemistry Page 1 CHAPTER 21 ELECTROCHEMISTRY 21-1. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO 3 ) 2 solution and a Cd(s) electrode submerged
More informationName AP CHEM / / Collected Essays Chapter 17 Answers
Name AP CHEM / / Collected Essays Chapter 17 Answers 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the
More informationCHM1 Review Exam 12. Topics REDOX
CHM1 Review Exam 12 Topics REDOX REDOX Reactions Oxidation Reduction Oxidizing agent Reducing agent Galvanic (Voltaic) Cells Anode Cathode Salt bridge Electrolyte Half-reactions Voltage o Positive voltages
More informationName Electrochemical Cells Practice Exam Date:
Name Electrochemical Cells Practice Exam Date: 1. Which energy change occurs in an operating voltaic cell? 1) chemical to electrical 2) electrical to chemical 3) chemical to nuclear 4) nuclear to chemical
More informationChapter 13: Electrochemistry. Electrochemistry. The study of the interchange of chemical and electrical energy.
Chapter 13: Electrochemistry Redox Reactions Galvanic Cells Cell Potentials Cell Potentials and Equilbrium Batteries Electrolysis Electrolysis and Stoichiometry Corrosion Prevention Electrochemistry The
More informationChapter 20. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 20 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The gain of electrons by an element is called. A) oxidation B) reduction C) sublimation
More informationRedox and Electrochemistry
Name: Thursday, May 08, 2008 Redox and Electrochemistry 1. A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from 1. the Pb(s) to the Cu(s) 2+
More informationELECTROCHEMICAL CELLS
1 ELECTROCHEMICAL CELLS Allessandra Volta (1745-1827) invented the electric cell in 1800 A single cell is also called a voltaic cell, galvanic cell or electrochemical cell. Volta joined several cells together
More informationAP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States
AP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States Chemical reactions in which the oxidation state of a substance changes are called oxidation-reduction reactions (redox reactions). Oxidation
More informationElectrochemistry. Chapter 18 Electrochemistry and Its Applications. Redox Reactions. Redox Reactions. Redox Reactions
John W. Moore Conrad L. Stanitski Peter C. Jurs http://academic.cengage.com/chemistry/moore Chapter 18 Electrochemistry and Its Applications Stephen C. Foster Mississippi State University Electrochemistry
More informationElectrochemistry Worksheet
Electrochemistry Worksheet 1. Assign oxidation numbers to each atom in the following: a. P 4 O 6 b. BiO 3 c. N 2 H 4 d. Mg(BrO 4 ) 2 e. MnSO 4 f. Mn(SO 4 ) 2 2. For each of the reactions below identify
More informationCELL POTENTIAL, E. Terms Used for Galvanic Cells. Uses of E o Values CELL POTENTIAL, E. Galvanic Cell. Organize halfreactions
Electrons move from anode to cathode in the wire. Anions & cations move thru the salt bridge. Terms Used for Galvanic Cells Galvanic Cell We can calculate the potential of a Galvanic cell using one of
More informationDiscovering Electrochemical Cells
Discovering Electrochemical Cells Part I Electrolytic Cells Many important industrial processes PGCC CHM 102 Cell Construction e e power conductive medium What chemical species would be present in a vessel
More informationPotassium ion charge would be +1, so oxidation number is +1. Chloride ion charge would be 1, so each chlorine has an ox # of -1
Chapter 18-1 1. Assign oxidation numbers to each atom in: Ni Nickel ion charge would be +2, so oxidation number is +2 Chloride ion charge would be 1, so each chlorine has an ox # of -1 Mg 2 Ti 4 Magnesium
More informationPreliminary Concepts. Preliminary Concepts. Class 8.3 Oxidation/Reduction Reactions and Electrochemistry I. Friday, October 15 Chem 462 T.
Class 8.3 Oxidation/Reduction Reactions and Electrochemistry I Friday, October 15 Chem 462 T. Hughbanks Preliminary Concepts Electrochemistry: the electrical generation of, or electrical exploitation of
More informationChemistry 122 Mines, Spring 2014
Chemistry 122 Mines, Spring 2014 Answer Key, Problem Set 9 1. 18.44(c) (Also indicate the sign on each electrode, and show the flow of ions in the salt bridge.); 2. 18.46 (do this for all cells in 18.44
More information4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?
HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm
More informationGalvanic cell and Nernst equation
Galvanic cell and Nernst equation Galvanic cell Some times called Voltaic cell Spontaneous reaction redox reaction is used to provide a voltage and an electron flow through some electrical circuit When
More informationGalvanic Cells. SCH4U7 Ms. Lorenowicz. Tuesday, December 6, 2011
Galvanic Cells SCH4U7 Ms. Lorenowicz 1 Electrochemistry Concepts 1.Redox reactions involve the transfer of electrons from one reactant to another 2.Electric current is a flow of electrons in a circuit
More informationCHAPTER 13: Electrochemistry and Cell Voltage
CHAPTER 13: Electrochemistry and Cell Voltage In this chapter: More about redox reactions Cells, standard states, voltages, half-cell potentials Relationship between G and voltage and electrical work Equilibrium
More informationReview: Balancing Redox Reactions. Review: Balancing Redox Reactions
Review: Balancing Redox Reactions Determine which species is oxidized and which species is reduced Oxidation corresponds to an increase in the oxidation number of an element Reduction corresponds to a
More informationPractical Examples of Galvanic Cells
56 Practical Examples of Galvanic Cells There are many practical examples of galvanic cells in use in our everyday lives. We are familiar with batteries of all types. One of the most common is the lead-acid
More informationElectrochemistry. Pre-Lab Assignment. Purpose. Background. Experiment 12
Experiment 12 Electrochemistry Pre-Lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. The questions should be answered
More informationUseful charge on one mole of electrons: 9.64 x 10 4 coulombs/mol e - = F F is the Faraday constant
Electrochemistry II: Cell voltage and Gibbs Free energy Reading: Moore chapter 19, sections 15.6-15.12 Questions for Review and Thought: 36, 40, 42, 44, 50, 54, 60, 64, 70 Key Concepts and Skills: definition
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationChapter 12: Oxidation and Reduction.
207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following
More informationNET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:
NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants
More informationAP* Chemistry ELECTROCHEMISTRY
Terms to Know: AP* Chemistry ELECTROCHEMISTRY the study of the interchange of chemical and electrical energy OIL RIG oxidation is loss, reduction is gain (of electrons) Oxidation the loss of electrons,
More informationEXPERIMENT 8: Activity Series (Single Displacement Reactions)
EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete
More informationSummer 2003 CHEMISTRY 115 EXAM 3(A)
Summer 2003 CHEMISTRY 115 EXAM 3(A) 1. In which of the following solutions would you expect AgCl to have the lowest solubility? A. 0.02 M BaCl 2 B. pure water C. 0.02 M NaCl D. 0.02 M KCl 2. Calculate
More informationCHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
More informationQuestion Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
More informationThe Electrical Control of Chemical Reactions E3-1
Experiment 3 The Electrical Control of Chemical Reactions E3-1 E3-2 The Task In this experiment you will explore the processes of oxidation and reduction, in which electrons flow between materials, and
More informationChemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
More informationChapter 21a Electrochemistry: The Electrolytic Cell
Electrochemistry Chapter 21a Electrochemistry: The Electrolytic Cell Electrochemical reactions are oxidation-reduction reactions. The two parts of the reaction are physically separated. The oxidation reaction
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationB) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
More informationBuilding Electrochemical Cells
Cautions Heavy metals, such as lead, and solutions of heavy metals may be toxic and an irritant. Purpose To determine the cell potential (E cell ) for various voltaic cells and compare the data with the
More informationIntroduction to electrolysis - electrolytes and non-electrolytes
Introduction to electrolysis - electrolytes and non-electrolytes Electrolysis is the process of electrically inducing chemical changes in a conducting melt or solution e.g. splitting an ionic compound
More informationMonatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
More information5.111 Principles of Chemical Science
MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. Page 1 of 10 pages
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationNomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula
Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationNomenclature of Ionic Compounds
Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.
More information12. REDOX EQUILIBRIA
12. REDOX EQUILIBRIA The electrochemical series (reference table) 12.1. Redox reactions 12.2. Standard electrode potentials 12.3. Calculations involving electrochemical cells 12.4. Using Eʅ values to predict
More informationChapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
More informationo Electrons are written in half reactions but not in net ionic equations. Why? Well, let s see.
REDOX REACTION EQUATIONS AND APPLICATIONS Overview of Redox Reactions: o Change in Oxidation State: Loses Electrons = Oxidized (Oxidation number increases) Gains Electrons = Reduced (Oxidation Number Reduced)
More informationFigure 1. A voltaic cell Cu,Cu 2+ Ag +, Ag. gas is, by convention, assigned a reduction potential of 0.00 V.
Voltaic Cells Introduction In this lab you will first prepare a set of simple standard half-cells and then measure the voltage between the half-cells with a voltmeter. From this data you will be able to
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationCHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
More information47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.
More informationHOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationExperiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
More informationGeneral Chemistry II Chapter 20
1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationInstructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
More information= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationNaming Compounds Handout Key
Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion
More informationElectrochemical Half Cells and Reactions
Suggested reading: Chang text pages 81 89 Cautions Heavy metals, such as lead, and solutions of heavy metals may be toxic and an irritant. Purpose To determine the cell potential (E cell ) for various
More informationDetermining Equivalent Weight by Copper Electrolysis
Purpose The purpose of this experiment is to determine the equivalent mass of copper based on change in the mass of a copper electrode and the volume of hydrogen gas generated during an electrolysis reaction.
More informationExperiment 9 Electrochemistry I Galvanic Cell
9-1 Experiment 9 Electrochemistry I Galvanic Cell Introduction: Chemical reactions involving the transfer of electrons from one reactant to another are called oxidation-reduction reactions or redox reactions.
More informationDecomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
More informationBalancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
More informationPeriodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationAPPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationChapter 2 Atoms, Ions, and the Periodic Table
Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More information5.111 Principles of Chemical Science
MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 26.1 5.111 Lecture
More informationCHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
More informationChapter 6 Oxidation-Reduction Reactions
65 Chapter 6 Oxidation-Reduction Reactions Review Skills 6.1 An Introduction to Oxidation-Reduction Reactions Oxidation, Reduction, and the Formation of Binary Ionic Compounds Oxidation-Reduction and Molecular
More informationCHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
More informationChemical Proportions in Compounds
Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of
More informationH 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.
CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More informationATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
More informationStudy Guide For Chapter 7
Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance
More informationMetals and Non-metals. Comparison of physical properties of metals and non metals
Metals and Non-metals Comparison of physical properties of metals and non metals PHYSICAL PROPERTY METALS NON-METALS Physical State Metallic lustre (having a shining surface) Mostly solids (Liquid -mercury)
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationA Review of the Construction of Electrochemical Cells
CHEM331 Physical Chemistry Revision 2.0 A Review of the Construction of Electrochemical Cells Electrochemical cells provide us with our first real example of a system which performs non-pv work. The work
More informationUNIT (4) CALCULATIONS AND CHEMICAL REACTIONS
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12
More informationNaming and Writing Formulas for Ionic Compounds Using IUPAC Rules
Naming and Writing Formulas for Ionic Compounds Using IUPAC Rules There are three categories of ionic compounds that we will deal with. 1.Binary ionic o simple ions (only single charges) o multivalent
More informationProblem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
More informationOxidation / Reduction Handout Chem 2 WS11
Oxidation / Reduction Handout Chem 2 WS11 The original concept of oxidation applied to reactions where there was a union with oxygen. The oxygen was either furnished by elemental oxygen or by compounds
More information